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Chapter 6: Problem 36

Draw three resonance structures for \(\mathrm{NO}_{3}^{-}\)

Short Answer

Expert verified
Three resonance structures are made for nitrate ion by displacing the double bond among the three oxygen atoms. These structures equally represent the molecule and are essentially an average of these possible resonant forms reflecting the behavior of the actual molecule.

Step by step solution

01

Drawing the primary structure

Start by drawing the primary Lewis structure. Nitrate ion (NO3-) consists of one nitrogen atom and three oxygen atoms, with a charge of -1. Nitrogen atom is the central atom and the oxygen atoms are surrounding it. Draw single bonds to connect N and O atoms. Also, add one extra electron to one of the oxygen atoms because of the -1 charge on the ion. Each oxygen atom will now have three lone pairs and the nitrogen atom will have no lone pairs.
02

Determining a resonance structure

A resonance structure of nitrate ion can be determined by moving one of the lone pairs from an oxygen atom to form a double bond with the nitrogen atom. Now this particular oxygen atom has two lone pairs and the nitrogen atom has one lone pair.
03

Drawing other resonance structures

Resonance happens because the molecule is not rigid but dynamic and the electrons can move freely. The initial structure is not the only one that can be drawn. Repeat step 2 for the other two oxygen atoms one by one. This provides us with two more resonance structures, making the total number of resonance structures for nitrate ion to be three.

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Most popular questions from this chapter

Name the following covalent compounds. a. \(\mathrm{SF}_{4}\) b. \(\mathrm{XeF}_{4}\) c. \(\mathrm{PBr}_{5}\) d. \(\mathrm{N}_{2} \mathrm{O}_{5}\) e. \(\mathrm{Si}_{3} \mathrm{N}_{4}\)

Why do electron pairs around a central atom stay as far apart as possible?

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